The number of `S^(2-)` ions present in `1L` of `0.1 MH_(2)S [K_(a(H_(2)S)) = 10^(-21)]` solution having `[H^(o+)] = 0.1M` is:

The number of S^(2-) ions present in 1 L of 0.1 (M) H_(2)S solution having [H^(+)]=0.1 (M) is ( Given H_(2)ShArr2H^(+)+S^(2-) K_(a)=1.1xx10^(-21) )

What is the maximum molarity of Co^(+2) ions in 0.1M HC1 saturated with 0.1M H_(2)S. (K_(a) = 4 xx 10^(-21)) . Given: K_(sp) of CoS = 2xx10^(-21) .

What is the maximum molarity of Co^(+2) ions in 0.1M HC1 saturated with 0.1M H_(2)S. (K_(a) = 4 xx 10^(-21)) . Given: K_(sp) of CoS = 2xx10^(-21) .

A solution contains 0.10 M H_2S and 0.3 HCl Calculate the concentration of S^(2-) and HS^(-) ions in the solution . For H_2S , K_(a_1) = 1 xx 10^(-7) and K_(a_2) = 1.3 xx 10^(-13)

A solution contains 0.1MH_(2) and 0.3MHCl. Calculate the concentration of S^(2) and HS- ions in the solution. For H_(2)S, K_(a_(1))=1.05xx10^(-7) and K_(a_(2))=1.3xx10^(-14) .

A solution containing both Zn^(2+) and Mn^(2+) ions at a concentration of 0.01M is saturated with H_(2)S . What is pH at which MnS will form a ppt ? Under these conditions what will be the concentration of Zn^(2+) ions remaining in the solution ? Given K_(sp) of ZnS is 10^(-22) and K_(sp) of MnS is 5.6 xx 10^(-16), K_(1) xx K_(2) of H_(2)S = 1.10 xx 10^(-21) .

A solution containing both Zn^(2+) and Mn^(2+) ions at a concentration of 0.01M is saturated with H_(2)S . What is pH at which MnS will form a ppt ? Under these conditions what will be the concentration of Zn^(2+) ions remaining in the solution ? Given K_(sp) of ZnS is 10^(-22) and K_(sp) of MnS is 5.6 xx 10^(-16), K_(1) xx K_(2) of H_(2)S = 1.10 xx 10^(-21) .